A robot spacecraft returned samples from the planetesimal 98765 ALEKS, located in the outer Solar System: Mass-spectroscopic analysis produced the following data on the isotopes of ruthenium in these samples: relative (amu) abundance mass isotope 101 Ru 100.9 91.5% 98 Ru 97.9 8.5% Use these measurements to complete the entry for ruthenium in the Periodic Table that would be used on 98765 ALEKS. Be sure your answers have the correct number of significant digits. Caution: your correct answer will have the same format but not necessarily the same numbers as the entry for ruthenium in the Periodic Table we use here on Earth. Ru 44 回山回国

A robot spacecraft returned samples from the planetesimal 98765 ALEKS, located in the outer Solar System: Mass-spectroscopic analysis produced the following data on the isotopes of ruthenium in these samples: relative (amu) abundance mass isotope 101 Ru 100.9 91.5% 98 Ru 97.9 8.5% Use these measurements to complete the entry for ruthenium in the Periodic Table that would be used on 98765 ALEKS. Be sure your answers have the correct number of significant digits. Caution: your correct answer will have the same format but not necessarily the same numbers as the entry for ruthenium in the Periodic Table we use here on Earth. Ru 44 回山回国

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter18: Nuclear Chemistry

Section: Chapter Questions

Problem 48QRT

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Similar questions

Which of the following are isotopes of element X, the atomic number for which is 9: 919X, 920X, 189X, and 921X?
2-102 An element consists of 90.51% of an isotope with a mass of 19.992 amu, 0.27% of an isotope with a mass of 20.994 amu, and 9.22% of an isotope with a mass of 21.990 amu. Calculate the average atomic mass and identify the element.
Verify that the atomic weight of magnesium is 24.31, given the following information: 24Mg, mass = 23.985042 u; percent abundance = 78.99% 25Mg, mass = 24.985837 u; percent abundance = 10.00% 26Mg, mass = 25.982593 u; percent abundance = 11.01%
How would you expect the chemical properties of isotopes of the same element to compare to each other? Explain your answer.
Where are neutrons found in an atom? Are neutrons positively charged, negatively charged, or electrically uncharged?
The following are properties of isotopes of two elements that are essential in our diet. Determine the number of protons, neutrons and electrons in each and name them. atomic number 26, mass number 58, charge of 2+ atomic number 53, mass number 127, charge of 1
2.84 Early attempts to arrange the elements often focused on atomic weight. Mendeleev considered a number of properties in addition to atomic weight, so he realized that some elements seemed out of place when ordered by atomic weight. Using the modern periodic table, identify elements for which Mendeleev must have had to switch the order in order to get the correct sequence of elements.
Slaters rules are a way to estimate the effective nuclear charge experienced by an electron. In this approach, the shielding constant, S, is calculated. The effective nuclear charge is then the difference between S and the atomic number, Z. (Note that the results in Table 7.2 and Figure 7.2 were calculated in a slightly different way.) Z = Z S The shielding constant, S, is calculated using the following rules: (1) The electrons of an atom are grouped as follows: (1s) (2s, 2p) (3s, 3p) (3d) (4s, 4p) (4d), and so on. (2) Electrons in higher groups (to the right) do not shield those in the lower groups. (3) For ns and np valence electrons a) Electrons in the same ns, np group contribute 0.35 (for 1s 0.30 works better). b) Electrons in n 1 groups contribute 0.85. c) Electrons in n 2 groups (and lower) contribute 1.00. (4) For nd and nf electrons, electrons in the same nd or nf group contribute 0.35, and those in groups to the left contribute 1.00. As an example, let us calculate Z for the outermost electron of oxygen: S = (2 0.85) + (5 0.35) = 3.45 Z = 8 3.45 = 4.55 Here is a calculation for a d electron in Ni: Z = 28 [18 1.00] [7 0.35] = 7.55 and for an s electron in Ni: Z = 28 [10 1.00] [16 0.85] [1 0.35] = 4.05 (Here 3s, 3p, and 3d electrons are in the (n 1) groups.) a) Calculate Z for F and Ne. Relate the Z values for O, F, and Ne to their relative atomic radii and ionization energies. b) Calculate Z for one of the 3d electrons of Mn, and compare this with Z for one of the 4s electrons of the element. Do the Z values give us some insight into the ionization of Mn to give the cation?
2.87 What is the heaviest element to have an atomic weight that is roughly twice its atomic number? What does this suggest must he true about the nuclei of atoms with higher atomic numbers?